Chem Q&A

This is the index for Chemistry Q&A videos developed by Dr. Glenn V. Lo, faculty colleagues (Ms. April Dupre, Dr. Vincent Giannamore, Ms. Cynthia Lamberty, and Dr. Jeremy Wessel) and students at Nicholls State University (Department of Physical Sciences). The development of most of these videos is funded through Project VALUE (Video Assessment Library for Undergraduate Education) by the Louisiana Board of Regents SELECT Grants Program (Contract No. LA-DL-SELECT-13-07/08). Other videos were developed by students for honors credit in Chemistry courses at Nicholls.


1-1 Differentiate hypothesis, observation, theory, and law, 1-2Differentiate physical states of matter in terms of shape, volume (compressibility), intermolecular distances, molecular motion, 1-3Describe separation techniques for samples of matter, 1-4Differentiate elements, compounds, and mixtures, 1-5 Write correct symbols for elements, 1-6 Classify elements based on their location in the periodic table, 1-7 Describe naturally-occurring forms of elements, 1-8 Describe the law of conservation of matter (mass), 1-9Describe and apply the law of definite composition, 1-10 Describe basic atomic structure (subatomic particles), 1-11 Interpret symbols for isotopes, 1-12 Describe how isotopes can be separated, 1-13Describe how the currently accepted model of the atom evolved from Dalton through Rutherford, 1-14 Describe how ions are formed from atoms, 1-15 Classify ions as cations or anions, 1-16 Interpret symbols and formulas of ions, 1-17 Predict stable monatomic ions formed from atoms, 1-18 Differentiate and predict ionic and covalent bonding, 1-19 Describe and differentiate molecules and polyatomic ions, 1-20 Interpret formulas of molecules and polyatomic ions, 1-21Classify polyatomic ions as oxoanions or non-oxoanions, 1-22Read/write formulas of polyatomic ions, 1-23 Classify compounds as molecular or ionic, 1-24 Write formulas of molecular and ionic compounds based on a description of the atoms or ions that make up a formula unit, 1-25 Differentiate ionic and molecular compounds in terms of physical properties, 1-26 Read and write formulas of binary compounds, 1-27 Read and write formulas of compounds containing polyatomic ions, 1-28 Read and write formulas of acids, 1-29 Describe and differentiate physical and chemical changes/properties, 1-30Identify reactants and products of a chemical reaction, 1-31 Construct a balanced chemical equation, 1-32 Classify and predict products of simple reactions

1A-1 Interpret SI prefixes, 1A-2 Identify significant figures in properly reported measurements, 1A-3 Relate uncertainty (precision) to how measurements are reported, 1A-4 Properly round off results of calculation involving measurements, 1A-5 Convert units, 1A-6Convert temperature readings, 1A-7 Convert temperature differences or changes, 1A-8 Solve problems dealing with measurements of physical properties (mass, volume, density, temperature, heat, heat capacity, solubility)

2-1 Describe electromagnetic radiation in terms of waves and photons, 2-2 Describe the Bohr model and relate to atomic spectra, 2-3 Describe orbitals and rules for assigning electrons to orbitals, 2-4Write or identify ground state and excited state electron configurations, 2-5 Relate (ground-state) electron configuration of an atom to its location in the periodic table, 2-6 Relate properties (size, ionization energy) of an atom to its location in the periodic table, 2-7Relate electron configuration and properties of ions to the parent atoms' location in the periodic table

3-1 Relate electronegativity to location of atom in the periodic table,3-2 Relate electronegativity and bond polarity, 3-3 Write and interpret Lewis dot symbols, 3-4 Interpret Lewis structures, 3-5 Draw Lewis structures, 3-6 Recognize and differentiate resonance and isomeric structures, 3-7 Determine formal charges, 3-8 Use formal charges and electronegativity to assess feasibility of a structure or extent of contribution to a resonance hybrid, 3-9 Recognize exceptions to the octet/duet rule, 3-10 Relate bond length to bond order and atomic sizes, 3-11 Describe molecular geometry using VSEPR, 3-12 Predict molecular polarity, 3-13 Describe intermolecular forces and relate to molecular structure and properties, 3-14 Use valence bond theory to explain molecular geometry, 3-15 Apply molecular orbital theory to diatomic molecules

4-1 Distinguish between masses of individual atoms and average masses, 4-2 Define mole and Avogadro number, 4-3 Relate mole count to individual count, 4-4 Count atoms and molecules in molecular compounds or ions in an ionic compound, 4-5 Relate moles and mass of pure substances, 4-6 Determine amount of element present in a compound, 4-7 Determine empirical and molecular formulas, 4-8Relate amounts of reactants and products in a chemical reaction, 4-9Determine limiting reactant and theoretical yield, 4-10 Determine amount of unreacted excess reactant

5-1 Differentiate solutions from compounds, 5-2 Differentiate solution, colloids, suspensions, and coarse mixtures, 5-3 Describe the dissolution of ionic and molecular compounds in water, 5-4 Classify solutions as saturated, supersaturated or unsaturated, 5-5 Classify ionic compounds as soluble or insoluble in water, 5-6 Recognize chemical equations for precipitation reactions, 5-7 Predict if a precipitation reaction could occur, 5-8 Write net ionic equations for precipitation reactions, 5-9 Describe strong and weak acids, 5-10Write chemical equations to represent ionization of acids in water, 5-11 Describe strong and weak bases, 5-12 Write chemical equations to represent acid-base reactions, 5-13 Write net ionic equations to represent acid-base reactions, 5-14 Calculate amount of solute given volume and molarity of solutions, 5-15 Calculate molarity of solutions and of ions in solution, 5-16 Solve dilution problems, 5-17 Solve stoichiometry problems involving solutions

6-1 Relate gas pressure to heights of liquid columns, 6-2 Relate Pressure, Volume, Temperature, and moles of gas, 6-3 Determine molar mass of a gas from density, Pressure, and Temperature data,6-4 Identify and apply empirical gas laws, 6-5 Apply Dalton's Law of partial pressures, 6-6 Solve stoichiometry problems involving gases,6-7 Interpret pressure and temperature in terms of molecular motion,6-8 Use Graham's law of effusion to compare effusion rates and determine molar mass of gas, 6-9 Describe and interpret real gas behavior, 6-10 Interpret one-component phase diagrams, 6-11Describe solid structure

7-1 Classify half reactions as reduction or oxidation, 7-2 Assign oxidation numbers, 7-3 Differentiate oxidation number from charge,7-4 Identify atoms oxidized or reduced based on oxidation numbers,7-5 Balance a redox reaction using oxidation number method, 7-6Balance redox half reactions in aqueous solution, 7-7 Construct a balanced redox reaction given two balanced half reactions